Solubility Multiple Choice
August 1998
13) In 0.20M Na2CrO4, the ion concentrations are
[Na+] / [CrO42-]A / 0.40M / 0.20M
B / 0.20M / 0.20M
C / 0.20M / 0.40M
D / 0.40M / 0.80M
14) Which of the following compounds is the least soluble in water?
A. H2S
B. KNO3
C. ZnSO4
D. Ca(OH)2
15) Which of the following 0.20M solutions will not form a precipitate when mixed with an equal volume of 0.20M Sr(OH)2?
A. CaS
B. NH4Cl
C. Na2SO4
D. Ba(NO3)2
16) Consider the following equilibrium:
SrF2(s) ⇄Sr2+ (aq) + 2F- (aq)
The equilibrium will shift left upon the addition of
A. H2O (l)
B. SrF2 (s)
C. SrCl2 (s)
D. NaNO3 (s)
17) Two ions found in hard water are Ca2+ and Mg2+. Which of the following will precipitate only one of these ions?
A. I-
B. S2-
C. SO42-
D. CO32-
18) At 25℃, the solubility of AgBr is
A. 2.9 × 10-25 M
B. 5.4 × 10-13 M
C. 2.7 × 10-13 M
D. 7.3 × 10-7 M
19) Which of the following saturated solutions has the greatest [CO32-]?
A. SrCO3
B. CaCO3
C. BaCO3
D. MgCO3
January 1999
14. Which of the following units could be used to describe solubility?
A. g/s B. g/L C. M/L D. mol/s
15. Consider the following anions:
When 10.0mL of 0.20M Pb(NO3) 2 are added to each of the above, precipitates form in:
A. I and II only.
B. I and III only.
C. II and III only.
D. I, II and III.
16. When equal volumes of 0.20M CuSO4 and 0.20M Li2S are combined, the complete
ionic equation is:
A. Cu 2+ (aq) + S2- (aq) ® CuS (s)
B. CuSO4 (aq) + Li2S (aq) ® CuS (s) + Li2SO4 (aq)
C. Cu 2+ (aq) +SO4 2- (aq) + 2Li + (aq) + S 2- (aq) ® Li2SO4 (aq) + CuS (s)
D. Cu 2+ (aq) +SO4 2- (aq) +2Li + (aq) +S 2- (aq) ® CuS (s) + 2Li + (aq) + SO4 2- (aq)
17. The Ksp expression for a saturated solution of Ag2CO3 is
A. Ksp = [Ag2+][CO32-]
B. Ksp = [Ag+ ]2[CO3-2]
C. Ksp = [2Ag+][CO3-2]
D. Ksp = [2Ag+]2[CO3-2]
18. The solubility of FeF2 is 8.4 ´10-3 M. The Ksp value is
A. 5.9 ´10-7
B. 2.4 ´10-6
C. 7.1´10-5
D. 8. 4 ´10-3
19. If the Trial Ion Product for AgBrO3 is calculated to be 1.0 ´10-7, then
A. a precipitate forms because the Trial Ion Product > Ksp
B. a precipitate forms because the Trial Ion Product < Ksp
C. no precipitate forms because the Trial Ion Product > Ksp
D. no precipitate forms because the Trial Ion Product < Ksp
20. The least soluble salt in water is
A. CaS
B. CaSO4
C. CaC2O4
D. Ca(NO3)2
April 1999
14. Which of the following produces a molecular solution when dissolved in water?
A. RbClO
B. CH3OH
C. NH4SCN
D. NaCH3COO
15. Consider the solubility equilibrium:
CaCO3(s) Ca2+(aq) + CO32-(aq)
An additional piece of solid CaCO3 is added to the equilibrium above.
The rate of dissolving and rate of crystallization have
16. At 25°C, which of the following compounds would dissolve to form
a saturated solution with the greatest [Pb2+]?
A. PbI2
B. PbCl2
C. PbBr2
D. Pb(IO3)2
17. When equal volumes of 0.20M ZnSO4 and 0.20M Sr(OH)2 are combined,
A. no precipitate forms.
B. a precipitate of only SrSO4 forms.
C. a precipitate of only Zn(OH)2 forms.
D. precipitates of both SrSO4 and Zn(OH)2 form.
18. The solubility of SnS is 3.2 ´10-3 M. The value of Ksp is
A. 1. 0 ´10-5
B. 3.2 ´10-3
C. 6.4 ´10-3
D. 5.7 ´10-2
19. Silver chloride, AgCl, would be least soluble in
A. 1.0M HCl
B. 1.0M NaNO3
C. 1.0M ZnCl2
D. 1.0M AgNO3
20. The solubility of SrF2 is
A. 4.3 ´10-9 M
B. 6.6 ´10-5 M
C. 1.0 ´10-3 M
D. 1.6 ´10-3 M
June 1999
14. The ion concentrations in 2.00L of 0.32M K3PO4 are
15. Which of the following compounds is the least soluble in water?
A. CaS
B. Fe (OH)3
C. KMnO4
D. NH4HC2O4
16. A solution contains two cations, each having a concentration of 0.20M. When an
equal volume of 0.20M OH- is added, these cations are removed from the solution by
precipitation. These ions are:
A. Ba2+ and K+
B. Sr2+ and Na+
C. Mg2+ and Sr2+
D. Mg2+ and Ca2+
17. The solubility of Mn(IO3)2 is 4.8 ´10-3 M. What is the value of Ksp ?
A. 1.1´10-7
B. 4.4 ´10-7
C. 7.1´10-6
D. 1.1´10-1
18. The maximum [SO42-] that can exist in 1.0 ´10-3 M Ca(NO3)2 without a precipitate
forming is:
A. 7.1´10-5 M
B. 1. 0 ´10-3 M
C. 8. 4 ´10-3 M
D. 7.1´10-2 M
August 1999
14. Consider the following solutes:
Which of the solutes above form only molecular aqueous solutions?
A. I and II
B. II and III
C. II, III and IV
D. I, II, III and IV
15. At a certain temperature, 7.0 ´10-4 mol MgSO4 is present in 100.0mL of solution.
The concentration of the Mg2+ in this solution is
A. 7.0 ´10-5 M
B. 7.0 ´10-4 M
C. 7.0 ´10-3 M
D. 7.0 ´10-6 M
16. When equal volumes of 0.20M SrBr2 and 0.20M AgNO3 are combined,
A. no precipitate forms.
B. a precipitate of only AgBr forms.
C. a precipitate of only Sr(NO3)2 forms.
D. precipitates of both AgBr and Sr(NO3)2 form.
17. Consider the following solubility equilibrium:
PbCl2 (s) Pb2+ (aq) + 2Cl- (aq)
A student adds NaCl (s) to a saturated solution of PbCl2 . When equilibrium is reestablished, how have the concentrations changed from the original equilibrium?
A. [Pb2+] and [Cl-] both increased.
B. [Pb2+] and [Cl-] both decreased.
C. [Pb2+] decreased and [Cl-] increased.
D. [Pb2+] increased and [Cl-] decreased.
18. Solid Ag2CrO4 is added to water to form a saturated solution. The Ksp value can be
calculated by:
A. Ksp = [CrO42-]2
B. Ksp = [CrO42-]3
C. Ksp = [CrO42-]3
2
D. Ksp = 4 [CrO42-]3
19. Consider the following solubility equilibrium:
BaSO3 (s) Ba2+(aq) + SO32- (aq)
Which of the following will result in an increase of [Ba2+] ?
A. adding water
B. adding BaS (s)
C. adding BaSO3 (s)
D. adding Na2SO3 (s)
20. When equal volumes of 0.20M Ca(NO3)2 and 0.20M Na2SO4 are combined,
A. a precipitate forms because Trial Ion Product > Ksp
B. a precipitate forms because Trial Ion Product < Ksp
C. no precipitate forms because Trial Ion Product > Ksp
D. no precipitate forms because Trial Ion Product < Ksp
21. Solid NaBrO3 is added to a 0.010M Ag+ solution. What is the [BrO3-] when a
precipitate first forms?
A. 2.8 ´10-9 M
B. 5.3 ´10-7 M
C. 5.3 ´10-3 M
D. 1. 0 ´10-2 M
January 2000
14. Which of the following does not define solubility?
A. the concentration of solute in a saturated solution
B. the moles of solute dissolved in a given volume of solution
C. the maximum mass of solute that can dissolve in a given volume of solution
D. the minimum moles of solute needed to produce one litre of a saturated solution
15. The ion concentrations in 0.25 M Al2(SO4)3 are
16. Which of the following will not produce a precipitate when equal volumes of 0.20 M
solutions are combined?
A. KOH and CaCl2
B. Zn(NO3)2 and K3PO4
C. Sr(OH)2 and (NH4)2S
D. Na2SO4 and Pb(NO3)2
17. What is observed when H2SO4 is added to a saturated solution of CaSO4?
A. the pH increases
B. the [Ca2+]increases
C. bubbles of H2 are given off
D. additional CaSO4 precipitates
18. The solubility of CdS = 2.8 x 10 -14 . The value of Ksp is
A. 7.8 x 10 -28
B. 2.8 x 10 -14
C. 5.6 x 10 -14
D. 1.7 x 10 -7
19. How many moles of solute are dissolved in 200.0 mL of a saturated solution of FeS?
A. 1.2 x 10 -19
B. 6.0 x 10 -19
C. 1.5 x 10 -10
D. 7.7 x 10 -10
20. Consider the following 10.0 mL solutions:
Equal moles of AgNO3 are added to each solution. It is observed that a precipitate forms in all but one solution. Which solution does not form a precipitate?
A. Cl-
B. Br -
C. IO3-
D. BrO3-
21. Which of the following could dissolve a precipitate of CaC2O4 in a saturated solution
of CaC2O4 ?
A. NaOH
B. CaC2O4
C. H2C2O4
D. Ca(NO3)2
April 2000
14. Which of the following will dissolve in water to produce a molecular solution?
A. CaCl2
B. NaOH
C. CH3OH
D. Sr(OH)2
15. In a solubility equilibrium, the
A. rate of dissolving equals the rate of crystallization.
B. neither dissolving nor crystallization are occurring.
C. concentration of solute and solvent are always equal.
D. mass of dissolved solute is greater than the mass of the solution.
16. Which of the following solutions would have [Fe+3] = 0.020 M ?
A. 0.40 L of 0.050 M Fe(NO3)3
B. 0.80 L of 0.020 M Fe2(SO4)3
C. 0.50 L of 0.040 M FeC6H5O7
D. 0.50 L of 0.010 M Fe2(C2O4)3
17. Which of the following substances has the lowest solubility?
A. BaS B. CuS C. FeS D. ZnS
18. The complete ionic equation for the reaction between MgS and Sr(OH)2 is
A. MgS(aq) + Sr(OH)2(aq) ® Mg(OH)2(s) + SrS(s)
B. MgS(aq) + Sr(OH)2(aq) ® Mg(OH)2(s) + SrS(aq)
C. Mg+2(aq) + S-2(aq) + Sr+2(aq) + 2OH-(aq) ® Mg+2(aq) + 2OH-(aq) + SrS(s)
D. Mg+2(aq) + S-2(aq) + Sr+2(aq) + 2OH-(aq) ® Mg(OH)2(s) + S-2(aq) + Sr+2(aq)
19. Consider the following equilibrium:
Fe(OH)2(s) Fe+2(aq) + 2OH-(aq)
Which of the following will cause the equilibrium to shift to the right?
A. adding KOH
B. adding Na2S
C. adding Fe(OH)2
D. adding Fe(NO3)2
20. Consider the following experiment:
The unknown solution could contain
A. 0.20 M OH-
B. 0.20 M NO3-
C. 0.20 M PO4-3
D. 0.20 M SO4-2
21. A compound has a solubility of 7.1 x 10-5 M at 25 °C. The compound is
A. CuS
B. AgBr
C. CaCO3
D. CaSO4
June 2000
14. A saturated solution of NaCl contains 36.5 g of solute in 0.100L of solution.
The solubility of the compound is
A. 0.062 M
B. 1.60 M
C. 3.65 M
D. 6.24 M
15. Calculate the [Li+] in 200.0 mL of 1.5 M Li2SO4
A. 0.30 M
B. 0.60 M
C. 1.5 M
D. 3.0 M
16. When equal volumes of 0.20 M RbCl and 0.20 M and M SrS are combined,
A. no precipitate forms.
B. a precipitate of Rb2S only forms.
C. a precipitate of SrCl2 only forms.
D. precipitates of both Rb2S and SrCl2 form.
17. A solution contains both Ag+ and Mg2+ ions. During selective precipitation, these
ions are removed one at a time by adding
A. I- followed by OH-
B. OH- followed by S2-
C. SO42- followed by Cl-
D. NO3- followed by PO43-
18. The Ksp expression for a saturated solution of Mg(OH)2 is
19. Consider the following saturated solutions:
CuSO4, BaSO4, CaSO4
The order of cation concentration, from highest to lowest, is
A. [Ba2+ ] > [Ca2+ ] > [Cu2+ ]
B. [Ca2+ ] > [Cu2+ ] > [Ba2+ ]
C. [Cu2+ ] > [Ca2+ ] > [Ba2+ ]
D. [Cu2+ ] > [Ba2+ ] > [Ca2+ ]
20. When 1.0 x10-3 moles of CuCl2 (s) are added to 1.0 L of 1.0 x10-3 M IO3-, the
A. Trial K sp > K sp and a precipitate forms.
B. Trial K sp < K sp and a precipitate forms.
C. Trial K sp > K sp and no precipitate forms.
D. Trial K sp < K sp and no precipitate forms.
August 2000
14. Which of the following forms a molecular solution in water?
A. SrSO4
B. Na3PO4
C. C6 H12O6
D. NH4CH3COO
15. Which of the following is necessary to form a saturated solution at equilibrium?
A. excess solute
B. an ionic solute
C. solute of low solubility
D. trial ion product is less than Ksp
16. The net ionic equation that describes a saturated solution of Ag2CrO4 is
A. Ag2CrO4 (s) Ag2CrO4 (aq)
B. Ag2CrO4 (s) 2Ag+ (aq) + CrO4–2 (aq)
C. Ag2CrO4 (s) 2Ag+ (aq) + Cr+6 (aq) + 4O-2 (aq)
D. 2Ag+ (aq) + CrO4–2 (aq) + 2H2O (l) 2AgOH (s) + H2CrO4 (aq)
17. Which of the following compounds has the lowest solubility?
A. SrS
B. CaCl2
C. Rb2CO3
D. Zn(OH)2
18. Which of the following will form a precipitate when equal volumes
of 0 2. M solutions are combined?
A. HI and Na2CO3
B. SrS and NH4OH
C. BaCl2 and CuSO4
D. Mg(NO3)2 and KCl
19. The solute AgBr is least soluble in
A. H2O
B. 1.0 M FeBr3
C. 1.0 M CaBr2
D. 1.0 M AgNO3
20. The magnesium and calcium ions in hard water can be removed by the addition of
A. NaI
B. NaNO3
C. Na2CO3
D. Na2SO4
21. The solubility of an AB2 type salt is 2.3 x 10–6 M. The salt is
A. PbBr2
B. Fe(OH)2
C. Cu(IO3) 2
D. Mg(OH)2
22. Which of the following saturated solutions will have the lowest [Pb2+]?
A. PbI2
B. PbCl2
C. Pb(IO3)2
D. Pb(NO3) 2
January 2001
14. A saturated solution forms when a 0.10 mol of salt is added to 1.0L of water.
The salt is
A. Li2S
B. CuBr2
C. Zn(OH)2
D. (NH4)2CO3
15. Consider the following equilibrium:
Ca(OH)2 (s) Ca+2 (aq) + 2OH- (aq)
Adding which of the following could cause the equilibrium [Ca+2] to increase?
A. H2O (l)
B. HCl (aq)